Chemistry Chapter 7-9
How many moles of K2 SO4 are in 15.0 g of K2 SO4 ? A) 0.172 moles B) 2.61 × 103 moles C) 0.111 moles D) 0.0861 moles E) 0.119 moles
D)
The ________ is the minimum energy needed for a chemical reaction to begin. A) reaction energy B) activation energy C) energy of reactants D) energy of products E) heat of reaction
B)
What is the classification for this reaction? SO3(g) + H2O (l) → H2SO4(l) A) decomposition B) combination C) replacement D) double replacement E) oxidation reduction
B)
When 3.05 moles of CH4 are mixed with 5.03 moles of O2 the limiting reactant is CH4 + 2O2 → CO2 + 2H2O A) CH4. B) O2. C) CO2. D) H2O.
B)
A chemical equation is balanced when A) the total number of molecules is the same in reactants and products. B) the total number of ions is the same in reactants and products. C) the sum of the coefficients of the reactants is equal to the sum of the coefficients of the products. D) the number of atoms of each element is the same in reactants and products. E) the charge on each atom is the same in reactants and products.
D)
For the reaction: 2H2O(l) + 137 kcal → 2H2 (g) + O2 (g), how many kcal are needed to react 50.0 g H2O(l)? A) 380. kcal B) 137 kcal C) 274 kcal D) 190. kcal E) 760. kcal
D)
How many molecules of water, H2O, are present in 75.0 g of H2O? A) 75.0 molecules B) 4.17 molecules C) 7.53 × 1024 molecules D) 2.51 × 1024 molecules E) 5.02 × 1024 molecules
D)
One mole of particles of any substance contains how many particles? A) 106 B) 3 × 10-10 C) 3 × 1010 D) 6.02 × 1023 E) 6.02 × 10-23
D)
What is the molar mass of copper(II) sulfate, CuSO4 ? A) 16.0 g B) 63.6 g C) 111.6 g D) 159.6 g E) 319.2 g
D)
When 4 moles of aluminum are allowed to react with an excess of chlorine gas, Cl2 , how many moles of aluminum chloride are produced? A) 1 mole B) 2 moles C) 3 moles D) 4 moles E) 5 moles
D)
Which of the following gives the balanced equation for this reaction? K3PO4 + Ca(NO3 )2 → Ca3 (PO4 )2 + KNO3 A) KPO4 + CaNO3 + KNO3 B) K3PO4 + Ca(NO3 )2 → Ca3 (PO4 )2 + 3KNO3 C) 2K3PO4 + Ca(NO3 )2 → Ca3 (PO4 )2 + 6KNO3 D) 2K3PO4 + 3Ca(NO3 )2 → Ca3 (PO4 )2 + 6KNO3 E) K3PO4 + Ca(NO3 )2 → Ca3 (PO4 )2 + KNO3
D)
0.50 mole of KCl is added to 2.0 kg of water. The boiling point of the solution will be ________ the boiling point of pure water. A) higher than B) lower than C) the same as
A)
An intravenous replacement solution contains 4.0 mEq/L of Ca2+ ions. How many grams of Ca2+ are in 3.0 L of the solution? A) 0.24 g B) 0.80 g C) 0.40 g D) 240 g E) 4.0 g
A)
During the process of diluting a solution to a lower concentration, A) the amount of solute does not change. B) the amount of solvent does not change. C) there is more solute in the concentrated solution. D) the volume of the solution does not change. E) water is removed from the concentrated solution.
A)
For the question(s) that follow, consider a 4% starch solution and a 10% starch solution separated by a semipermeable membrane. Which starch solution will decrease in volume as osmosis occurs? A) 4% B) 10% C) Neither exerts osmotic pressure. D) They exert equal osmotic pressures. E) They exert opposite osmotic pressures.
A)
Hydrogen bonds are a major factor in the structure of A) DNA. B) hydrogen chloride. C) dry ice. D) air. E) table salt.
A)
The molarity (M) of a solution refers to A) moles of solute/L of solution. B) moles of solute/L of solvent. C) moles of solute/100 mL of solution. D) grams of solute/100 mL of solution. E) grams of solute/L of solution.
A)
What is the molarity of a solution containing 5.0 moles of KCl in 2.0 L of solution? A) 2.5 M B) 1.0 M C) 5.0 M D) 10. M E) 2.0 M
A)
When solutions of NaCl and AgNO3 are mixed, A) a precipitate of AgCl forms. B) a precipitate of NaNO3 forms. C) no precipitate forms. D) precipitate of NaNO3 and AgCl form. E) a precipitate of AgCl2 forms.
A)
What is the molarity of a solution that contains 17 g of NH3 in 0.50 L of solution? A) 34 M B) 2.0 M C) 0.50 M D) 0.029 M E) 1.0 M
B
1.0 mole of NaCl is added to 1.0 kg of water. The freezing point of the solution will be ________ the freezing point of pure water. A) higher than B) lower than C) the same as
B)
A homogeneous mixture that does not settle out upon standing is A) an element. B) a colloid. C) a suspension. D) homogeneous. E) hydrated.
B)
For the question(s) that follow, consider a 4% starch solution and a 10% starch solution separated by a semipermeable membrane. Which of the following occurs in this system? A) Water flows equally in both directions. B) There is a net flow of water from the 4% starch solution into the 10% starch solution. C) There is a net flow of water from the 10% starch solution into the 4% starch solution. D) Water does not cross the membrane at all. E) Starch moves out of the 10% starch solution into the 4% starch solution.
B)
How many equivalents are present in 5.0 g of Al3+? A) 15 Eq B) 0.56 Eq C) 0.19 Eq D) 0.37 Eq E) 3 Eq
B)
How many grams of barium chloride are needed to make 100. grams of barium sulfate? A) 44.9 g B) 89.2 g C) 208.3 g D) 233.3 g E) 46.6 g
B)
How many grams of glucose (C6H12O6 ) are in 3.55 moles of glucose? A) 180. g B) 639 g C) 103 g D) 426 g E) 50.7 g
B)
If 100. mL of water is added to 25 mL of 5.0 M NaCl, the final concentration is ________. A) 25 M B) 1.0 M C) 5.0 M D) 2.0 M E) 1.3 M
B)
In this reaction, what is the correct coefficient for hydrogen gas? ? H2 + ? O2 → ? H2O A) 1 B) 2 C) 3 D) 4 E) 5
B)
Oil does not dissolve in water because A) oil is polar. B) oil is nonpolar. C) water is nonpolar. D) water is saturated. E) oil is hydrated.
B)
What is the molarity of a KCl solution made by diluting 75.0 mL of a 0.200 M solution to a final volume of 100. mL? A) 0.267 M B) 0.150 M C) 0.200 M D) 6.67 M E) 0.100 M
B)
What type of reaction is: CH4 + 2O2 → CO2 + 2H2O + 218 kcal? A) an endothermic reaction B) an exothermic reaction C) a single replacement reaction D) a combination reaction E) a decomposition reaction
B)
What volume of a 2.00 M KCl solution is required to prepare 500. mL of a 0.100 M KCl solution? A) 0.0400 mL B) 25.0 mL C) 2.00 mL D) 1.00 × 104 mL E) 5.00 × 102 mL
B)
When 200. mL of water are added to 100. mL of 12% KCl solution the final concentration of KCl is (Assume the volumes add.) A) 12%. B) 4.0%. C) 36%. D) 6.0%. E) 8.0%.
B)
2Mg + O 2 → 2MgO2 ) The number of moles of MgO produced when 0.20 mole of O2 reacts completely is A) 0.10 mole. B) 0.20 mole. C) 0.40 mole. D) 0.60 mole. E) 0.80 mole.
C)
A mixture in which one component settles is called a(n) ________. A) solution B) colloid C) suspension D) electrolyte E) nonelectrolyte
C)
Acetic acid can be classified as a(n) ________. A) gas B) solid C) weak electrolyte D) strong electrolyte E) ionic compound
C)
An increase in the temperature of a solution usually A) increases the boiling point. B) increases the solubility of a gas in the solution. C) increases the solubility of a solid solute in the solution. D) decreases the solubility of a solid solute in the solution. E) decreases the solubility of a liquid solute in the solution.
C)
Find the mass of AlCl3 that is produced when 25.0 grams of Al2O3 react with excess HCl according to the following equation. Al2O3(s) + 6HCl(aq) → 2AlCl3(aq) + 3H2O(l) A) 155 g B) 72.9 g C) 65.4 g D) 32.6 g E) 16.3 g
C)
How many grams of PbCl2 are formed when 25.0 mL of 0.654 M KCl react with Pb(NO3)2? 2KCl(aq) + Pb(NO3) 2(aq) → 2KNO3(aq) + PbCl2(s) A) 22.7 g B) 1.64 g C) 2.27 g D) 4.54 g E) 9.08 g
C)
How many grams of barium sulfate can be produced from 20.8 g of barium chloride? A) 1.37 g B) 2.33 g C) 23.3 g D) 137 g E) 233 g
C)
How many grams of glucose are needed to prepare 400. mL of a 2.0%(m/v) glucose solution? A) 800. g B) 0.0050 g C) 8.0 g D) 2.0 g E) 200. g
C)
In a solution, the solvent A) is a liquid. B) can be a liquid or gas. C) can be a solid, liquid, or gas. D) is never a solid. E) is the substance present in the smallest concentration.
C)
The molarity of a solution of 5.0 g of KCl in 100. mL of solution is ________. A) 0.038 M B) 0.067 M C) 0.67 M D) 0.13 M E) 1.3 M
C)
Use the reaction: 2AgNO3(aq) + H2SO4(aq) → Ag2SO4(s) + 2H2O(l). What volume of 0.123 M AgNO3(aq) is needed to form 0.657 g of Ag2SO4(s)? A) 34.2 L B) 17.1 mL C) 34.3 mL D) 10.7 mL E) 53.4 mL
C)
Water is a polar solvent and hexane (C6H14) is a nonpolar solvent. Which of the following correctly describes the solubility of the solute? A) mineral oil, soluble in water B) CaCl2, soluble in hexane C) NaHCO3, soluble in water D) CCl4, soluble in water E) octane, soluble in water
C)
What is the coefficient for carbon dioxide in the balanced equation? A) 2 B) 4 C) 5 D) 6 E) 8
C)
What volume of 0.10 M NaOH can be prepared from 250. mL of 0.30 M NaOH? A) 0.075 L B) 0.25 L C) 0.75 L D) 0.083 L E) 750 L
C)
What volume of a 1.5 M KOH solution is needed to provide 3.0 moles of KOH? A) 3.0 L B) 0.50 L C) 2.0 L D) 4.5 L E) 0.22 L
C)
Which of the following molecules can form hydrogen bonds? A) CH4 B) NaH C) NH3 D) BH3 E) HI
C)
Which one of the following compounds will NOT be soluble in water? A) LiOH B) K2S C) BaSO4 D) NaNO3 E) MgCl2
C)
Which one of the following compounds will be soluble in water? A) AgBr B) Cu(OH)2 C) NH4Cl D) CaCO3 E) PbS
C)
Which one of the following compounds will be soluble in water? A) AgCl B) Cu(OH)2 C) LiCl D) CaSO4 E) PbCO3
C)
How many moles of CaCl2 are in 250 mL of a 3.0 M of CaCl2 solution? A) 750 moles B) 1.3 moles C) 83 moles D) 0.75 mole E) 3.0 moles
D)
In the process known as osmosis, ________ moves through a semipermeable membrane into an area of ________ concentration. A) solute; lower solute B) solute; higher solute C) solvent; lower solute D) solvent; lower solvent E) solvent; higher solvent
D)
NaCl can be classified as a ________. A) gas B) liquid C) weak electrolyte D) strong electrolyte E) nonelectrolyte
D)
What is the coefficient for water in the balanced equation? A) 2 B) 4 C) 5 D) 6 E) 8
D)
What is the concentration, in mass percent, of a solution prepared from 50.0 g NaCl and 150.0 g of water? A) 0.250% B) 33.3% C) 40.0% D) 25.0% E) 3.00%
D)
What is the osmolarity of a solution made by dissolving 25.0 g of the strong electrolyte KCl in 1.0 L of solution? A) 0.168 Osm B) 0.335 Osm C) 0.250 Osm D) 0.670 Osm E) 1.34 Osm
D)
When solutions of KCl and Pb(NO3)2 are mixed, a precipitate forms. Which of the following is the balanced equation for the double replacement reaction that occurs? A) KCl(aq) + Pb(NO3) 2(aq) → KNO3(aq) + PbCl2(s) B) KNO3(aq) + PbCl2(s) → KCl(aq) + Pb(NO3) 2(aq) C) K+(aq) + NO3-(aq) → KNO3(aq) D) 2KCl (aq) + Pb(NO3)2(aq) → 2KNO3(aq) + PbCl2 (s) E) KCl(aq) + Pb(NO3)2(aq) → KNO3(aq) + PbCl(s)
D)
) A red blood cell will undergo crenation in A) water. B) 0.5% NaCl. C) 3% glucose. D) 5% glucose. E) 7% NaCl.
E)
0.50 mole of NaCl is added to 1.0 kg of water. The freezing point of the solution will be ________. A) 0.00 °C B) 0.93 °C C) 1.86 °C D) -0.93 °C E) -1.86 °C
E)
Rubbing alcohol is 70.% isopropyl alcohol by volume. How many mL of isopropyl alcohol are in a 1 pint (473 mL) container? A) 70. mL B) 0.15 mL C) 680 mL D) 470 mL E) 330 mL
E)
Using a kidney machine to remove waste products from the blood is known as ________. A) osmosis B) osmolysis C) autolysis D) hemolysis E) hemodialysis
E)
Which of the following correctly gives the best coefficients for the reaction below? N2H4+ H2O2 → N2+ H2O A) 1, 1, 1 ,1 B) 1, 2, 1, 4 C) 2, 4, 2, 8 D) 1, 4, 1, 4 E) 2, 4, 2, 4
B)
For the reaction: 2H2O(l) + 137 kcal → 2H2 (g) + O2 (g), how many kcal are needed to form 2.00 moles O2 (g)? A) 68.5 kcal B) 137 kcal C) 274 kcal D) 190. kcal E) 548 kcal
C)
How many atoms of neon are present in 1.30 moles of neon? A) 3.15 × 1023 atoms B) 4.63 × 1023 atoms C) 7.83 × 1023 atoms D) 6.02 × 1023 atoms E) 7.83 × 1024 atoms
C)
How many grams of hydrogen are needed to produce 1.80 g of water according to this equation? 2H2 + O2 → 2H2O A) 0.100 g B) 0.180 g C) 0.200 g D) 2.00 g E) 4.00 g
C)
How many kcal are produced when 32.0 g of CH4 react? CH4 + 2O2 → CO2 + 2H2O + 218 kcal A) 218 kcal B) 109 kcal C) 436 kcal D) 6.81 kcal
C)
In the reaction of nitrogen gas, N2 , with hydrogen gas, H2 , to form ammonia gas, NH3 , how many moles of hydrogen are needed to react with two moles of nitrogen? A) 2 moles B) 4 moles C) 6 moles D) 8 moles E) 10 moles
C)
The reaction of carbon with oxygen to produce carbon monoxide is an example of which class of reaction? 2C(s) + O2(g) → 2CO(g) A) single replacement B) double replacement C) combination D) catalytic E) endothermic
C)
3.00 moles of NO2 have a mass of A) 138 g. B) 46.0 g. C) 30.0 g. D) 90.0 g. E) 45.0 g.
A)
Any reaction that absorbs 150 kcal of energy can be classified as A) endothermic. B) exothermic. C) activated. D) reduction. E) oxidation.
A)
Calculate the molar mass of potassium chloride, KCl. A) 74.6 g B) 54.5 g C) 6.74 g D) 67.4 g E) 19.0 g
A)
What is oxidized and what is reduced in the following reaction? 2Al(s) + 3Br2 (g) → 2AlBr3 (s) A) Al is oxidized and Br2 is reduced. B) AlBr3 is reduced and Br2 is oxidized. C) Al is reduced and Br2 is oxidized. D) AlBr3 is reduced and Al is oxidized. E) AlBr3 is oxidized and Al is reduced.
A)
Calculate the molar mass of magnesium chloride, MgCl2 . A) 24.3 g B) 95.2 g C) 125.9 g D) 59.8 g E) 70.0 g
B)
4.00 moles of sodium have a mass of A) 4.60 g. B) 11.0 g. C) 23.0 g. D) 44.0 g. E) 92.0 g.
E)
In a ________ reaction, two or more elements or compounds form one product. A) decomposition B) single replacement C) dehydration D) double replacement E) combination
E)
The ________ is the energy difference between reactants and products in a chemical reaction. A) transition energy B) activation energy C) product energy D) overall energy E) heat of reaction
E)
What is the molar mass of Mg3 (PO4 )2 , a substance formerly used in medicine as an antacid? A) 71.3 g B) 118 g C) 150. g D) 214 g E) 263 g
E)
The number of particles in 1 mole of hydrogen gas is ________.
6.02 × 1023
A hydrogen bond is A) an attraction between a hydrogen atom attached to N, O, or F and an N, O, or F atom on another molecule. B) a covalent bond between H and O. C) an ionic bond between H and another atom. D) a bond that is stronger than a covalent bond. E) the polar O-H bond in water.
A)
A patient needs to receive 85 grams of glucose every 12 hours. What volume of a 5.0%(m/v) glucose solution needs to be administered to the patient each 12 hours? A) 1700 mL B) 60 mL C) 6000 mL D) 17 mL E) 204 mL
A)
A red blood cell will undergo hemolysis in A) water. B) 0.9% NaCl. C) 5% glucose. D) 5% NaCl. E) 10% glucose.
A)
A solution with the same osmotic pressure as the blood is A) isotonic to the blood. B) hypotonic to the blood. C) hypertonic to the blood. D) nontonic to the blood. E) molar to the blood.
A)
An aqueous mixture containing starch (a colloid), NaCl, glucose, and albumin (a colloid) is placed in a dialyzing bag and immersed in distilled water. Which of the following correctly describes the location of the indicated substance after dialysis? A) albumin, inside B) starch outside C) albumin inside and outside D) water inside only E) starch inside and outside
A)
How many equivalents are present in 5.0 moles of Al3+? A) 15 Eq B) 1.3 Eq C) 5.0 Eq D) 0.67 Eq E) 3.0 Eq
A)
In water, a substance that partially ionizes in solution is called a A) weak electrolyte. B) nonelectrolyte. C) semiconductor. D) nonconductor. E) strong electrolyte.
A)
What is the new mass/volume (m/v)% of a KOH solution that is prepared by diluting 110 mL of a 6% (m/v) KOH solution to 330 mL? A) 2% B) 1% C) 6% D) 12% E) 18%
A)
A reaction that releases energy as it occurs is classified as a(n) A) endothermic reaction. B) exothermic reaction. C) oxidation-reduction reaction. D) catalyzed reaction. E) decomposition reaction.
B)
A solution is prepared by dissolving 2 g of KCl in 100 g of H2O. In this solution, H2O is the A) solute. B) solvent. C) solution. D) solid. E) ionic compound.
B)
According to Henry's law, the solubility of a gas in a liquid A) decreases as the gas pressure above the liquid increases. B) increases as the gas pressure above the liquid increases. C) remains the same as the temperature increases. D) depends on the liquid polarity. E) depends on the liquid density.
B)
How many moles of barium sulfate are produced from 0.100 mole of barium chloride? A) 0.0100 mole B) 0.100 mole C) 0.200 mole D) 1.00 mole E) 2.00 moles
B)
How many moles of carbon atoms are there in 0.500 mole of C2H6 ? A) 0.500 moles B) 1.00 moles C) 3.00 moles D) 6.02 × 1023 moles E) 4.00 moles
B)
In the following reaction, when the equation is correctly balanced, what is the correct coefficient for sodium chloride? Pb(NO3)2(aq) + NaCl(aq) → PbCl2(s) + NaNO3(aq) A) 1 B) 2 C) 3 D) 4 E) 5
B)
The O-H bond in water is polar because A) it is an ionic bond. B) oxygen is much more electronegative than hydrogen. C) oxygen occupies more space than hydrogen. D) hydrogen is much more electronegative than oxygen. E) it is a hydrogen bond.
B)
The process by which a semipermeable membrane allows water molecules, small molecules, and ions to pass through while retaining large particles is called A) osmotic pressure. B) dialysis. C) solvation. D) dilution. E) hydration.
B)
What is the concentration, in m/v percent, of a solution prepared from 50. g NaCl and 2.5 L of water? A) 5.0% B) 2.0% C) 0.020% D) 0.050% E) 20.%
B)
Which one of the following compounds will NOT be soluble in water? A) NaOH B) PbS C) K2SO4 D) LiNO3 E) MgCl2
B)
An equivalent is A) the amount of ion that has a 1+ charge. B) the amount of ion that has a 1- charge. C) the amount of ion that carries 1 mole of electrical charge. D) 1 mole of any ion. E) 1 mole of an ionic compound.
C)
Find the mass of AlCl3 that is produced when 10.0 grams of Al2O3 react with 10.0 g of HCl according to the following equation. Al2O3(s) + 6HCl(aq) → 2AlCl3(aq) + 3H2O(aq) A) 16.2 g B) 20.0 g C) 12.2 g D) 10.0 g E) 6.10 g
C)
In the reaction of silver nitrate with sodium chloride, how many grams of silver chloride will be produced from 100. g of silver nitrate when it is mixed with an excess of sodium chloride? The equation for the reaction is below. AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) A) 107.9 g B) 169.9 g C) 84.4 g D) 0.589 g E) 58.9 g
C)
The molar mass of calcium hydroxide, Ca(OH)2 , is A) 58.1 g. B) 57.1 g. C) 74.1 g. D) 114.2 g. E) 38.0 g.
C)
(Q) What coefficient is placed in front of O2 to complete the balancing of the following equation? C5H8+ ? O2 → 5CO2 + 4H2O A) 1 B) 3 C) 5 D) 7 E) 9
D)
A solution that has an osmotic pressure less than that of red blood cells is called A) saturated. B) hypertonic. C) isotonic. D) hypotonic. E) unsaturated.
D)
How many equivalents are present in 0.40 moles of SO4 2-? A) 0.10 Eq B) 0.20 Eq C) 0.40 Eq D) 0.80 Eq E) 1.2 Eq
D)
How many grams of CO2 are produced from 125 g of O2 and excess CH4? CH4 + 2O2 → CO2 + 2H2O A) 125 g of CO2 B) 62.5 g of CO2 C) 172 g of CO2 D) 85.9 g of CO2 E) 250. g of CO2
D)
How many grams of H2O are needed to produce 150 g of Mg(OH)2? A) 46 g B) 18 g C) 130 g D) 93 g E) 23 g
D)
The mass percent concentration refers to A) grams of solute in 1 kg of solvent. B) grams of solute in 1 kg of solution. C) grams of solute in 100 g of solvent. D) grams of solute in 100 g of solution. E) grams of solvent in 100 g of solution.
D)
The mass/volume percent concentration refers to A) grams of solute in 1 L of solvent. B) grams of solute in 1 L of solution. C) grams of solute in 100 mL of solvent. D) grams of solute in 100 mL of solution. E) grams of solvent in 100 mL of solution.
D)
The molar mass of potassium is A) 19 g. B) 31.0 g. C) 6.02 × 1023 grams. D) 39.1 g. E) 15g.
D)
The reaction of methane with oxygen to produce carbon dioxide and water is an example of which class of reaction? CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) A) single replacement B) double replacement C) combination D) oxidation E) endothermic
D)
The solubility of KI is 50 g in 100 g of H2O at 20 °C. If 110 grams of KI are added to 200 grams of H2O A) all of the KI will dissolve. B) the solution will freeze. C) the solution will start boiling. D) a saturated solution will form. E) the solution will be unsaturated.
D)
What is the molarity of a solution that contains 3.25 moles of NaNO3 in 250. mL of solution? A) 3.25 M B) 6.50 M C) 0.0130 M D) 13.0 M E) 2.60 M
D)
What is the molarity of a solution which contains 58.5 g of sodium chloride dissolved in 0.500 L of solution? A) 0.500 M B) 1.00 M C) 1.50 M D) 2.00 M E) 4.00 M
D)
When KCl dissolves in water A) the Cl- ions are attracted to dissolved K+ ions. B) the Cl- ions are attracted to the partially negative oxygen atoms of the water molecule. C) the K+ ions are attracted to Cl- ions on the KCl crystal. D) the K+ ions are attracted to the partially negative oxygen atoms of the water molecule. E) the K+ ions are attracted to the partially positive hydrogen atoms of the water molecule.
D)
When some of the sugar added to iced tea remains undissolved at the bottom of the glass, the solution is A) dilute. B) polar. C) nonpolar. D) saturated. E) unsaturated.
D)
Which one of the following compounds will be insoluble in water? A) AgNO3 B) CaCl2 C) NH4Cl D) CaCO3 E) Pb(C2H3O2)2
D)
Which solution is isotonic to a red blood cell? A) water B) 0.5% NaCl C) 2% glucose D) 0.9% NaCl E) 10% glucose
D)
1.25 moles of PbO2 have a mass of A) 191 g. B) 279 g. C) 178 g. D) 239 g. E) 299 g.
E)
For the question(s) that follow, consider a 4% starch solution and a 10% starch solution separated by a semipermeable membrane. The process that occurs in this system is A) filtration. B) hydration. C) neutralization. D) dialysis. E) osmosis.
E)
How many mL of 0.246 M Pb(NO3)2 are needed to react with 36.0 mL of 0.322 M KCl ? 2KCl(aq) + Pb(NO3) 2(aq) → 2KNO3(aq) + PbCl2(s) A) 36.0 mL B) 18.0 mL C) 72.0 mL D) 47.1 mL E) 23.6 mL
E)
How many milliliters of a 25% (m/v) NaOH solution would contain 75 g of NaOH? A) 25 mL B) 75 mL C) 33 mL D) 19 mL E) 3.0 × 102 mL
E)
How many moles of hydrogen peroxide (H2O2) are needed to produce 5.0 moles of water? A) 1.0 mole B) 2.0 moles C) 4.0 moles D) 5.0 moles E) 8.0 moles
E)
In water, a substance that ionizes completely in solution is called a A) weak electrolyte. B) nonelectrolyte. C) semiconductor. D) nonconductor. E) strong electrolyte.
E)
Methanol, CH3OH, can be classified as a ________. A) gas B) solid C) weak electrolyte D) strong electrolyte E) nonelectrolyte
E)
What is the osmolarity of a solution made by dissolving 0.50 mole of the strong electrolyte CaCl2 in 1.0 L of solution? A) 0.50 Osm B) 1.0 Osm C) 1.5 Osm D) 2.0 Osm E) 0.0 Osm
E)
What volume (mL) of a 15% (m/v) NaOH solution contains 120 g NaOH? A) 18 mL B) 0.13 mL C) 13 mL D) 120 mL E) 8.0 × 102 mL
E)
What volume of 2.5% (m/v) KOH can be prepared from 125 mL of a 5.0% KOH solution? A) 0.0040 mL B) 63 mL C) 0.10 mL D) 125 mL E) 250 mL
E)
What type of reaction is the following? Zn + 2HCl → ZnCl2 + H2
single replacement reaction
The molar mass of C3H8O2 is A) 76.0 g. B) 60.0 g. C) 29.0 g. D) 69.0 g. E) 52.0 g.
A)
One mole of helium gas has a mass of A) 1.00 g. B) 2.00 g. C) 3.00 g. D) 4.00 g. E) 8.00 g.
D)
What is the coefficient of hydrogen, H2 , when the following equation is balanced? Al + H2SO4 → Al2(SO4)3+ ? H2 A) 1 B) 2 C) 3 D) 4 E) 5
C)
What is the molar mass of sodium phosphate, Na3PO4 ? A) 119 g B) 308 g C) 164 g D) 226 g E) 354 g
C)
When 60.0 g of CH4 reacts with excess O2, the actual yield of CO2 is 112 g. What is the percent yield? CH4 + 2O2 → CO2 + 2H2O A) 53.6 % B) 187 % C) 67.9 % D) 46.4 %
C)
Which of the following is an oxidation-reduction reaction? A) CaCl2+ Na2SO4 → CaSO4+ 2NaCl B) KOH + HNO3 → H2O + KNO3 C) N2 + O2 → 2NO D) AgNO3+ NaCl → AgCl + NaNO3 E) Al2(SO4)3 + 6KOH → 2Al(OH)3+ 3K2SO4
C)
0.100 mole of lithium has a mass of A) 3.00 g. B) 0.300 g. C) 6.94 g. D) 0.694 g. E) 0.700 g.
D)
2Mg + O2 → 2MgO How many grams of MgO are produced when 40.0 grams of O2 react completely with Mg? A) 30.4 g B) 50.4 g C) 60.8 g D) 101 g E) 201 g
D)
Avogadro's number is the number of A) particles in 1 mole of a substance. B) amu in 1 mole of a substance. C) grams in 1 mole of a substance. D) moles in 6.02 × 1023 grams of an element. E) moles in 6.02 × 1023 amu of an element.
A)
How many grams of Fe2O3 are there in 0.500 mole of Fe2O3 ? A) 79.9 g B) 35.9 g C) 63.8 g D) 51.9 g E) 160. g
A)
How many grams of NO are required to produce 145 g of N2 in the following reaction? 4NH3(g) + 6NO(g) → 5N2(g) + 6H2O(l) A) 186 g B) 155 g C) 125 g D) 129 g E) 145 g
A)
How many moles of magnesium are needed to react with 0.50 mole of O2 ? A) 0.50 mole B) 1.0 moles C) 2.0 moles D) 3.0 moles E) 4.0 moles
B)
How many moles of water, H2O, are present in 75.0 g of H2O? A) 4.41 moles B) 4.16 moles C) 75.0 moles D) 7.50 moles E) 1.35 × 103 moles
B)
If the reaction shown below is exothermic, the energy level of the reactants is H2 + O2 → 2H2O A) lower than that of the products. B) higher than that of the products. C) the same as that of the products. D) possibly lower, possibly higher than that of the products. E) higher than the activation energy of the reaction.
B)
In an endothermic reaction A) heat flows out of the system. B) energy is absorbed by the system. C) the temperature of the system increases. D) the products have less energy that the reactants. E) the products have the same energy that the reactants.
B)
In an oxidation-reduction reaction, the substance oxidized always A) takes on oxygen atoms. B) shows a loss of electrons. C) gives up hydrogen atoms. D) shows a gain of electrons. E) becomes a charged species.
B)
In any balanced chemical equation, the number of each type of atom on both sides of the equation is A) doubled. B) the same. C) decreased by one. D) increased by one. E) dependent on the temperature.
B)
How many grams of hydrogen peroxide (H2O2) are needed to produce 25.0 g of oxygen? A) 106 g B) 26.6 g C) 5.88 g D) 25.0 g E) 53.1 g
E)
How many hydrogen atoms are present in 75.0 g of H2O? A) 75.0 atoms B) 4.17 atoms C) 7.53 × 1024 atoms D) 2.51 × 1024 atoms E) 5.02 × 1024 atoms
E)
Pentane (C5H12) reacts with oxygen (O2) to form carbon dioxide (CO2) and water (H2O) according to thefollowing reaction. Answer the question(s) that follow about this reaction. C5H12 + ? O2 → ? CO2+ ? H2O What is the coefficient for oxygen in the balanced equation? A) 2 B) 4 C) 5 D) 6 E) 8
E)
In the following reaction, when the equation is correctly balanced, what is the correct coefficient for aluminum chloride? Al(s) + Cl2(g) → AlCl3(s) A) 1 B) 2 C) 3 D) 4 E) 5 Answer:
B)
Which of the following describes an oxidation reaction? A) loss of electrons or loss of oxygen B) loss of electrons or gain of oxygen C) loss of electrons or gain of hydrogen D) gain of electrons or gain of oxygen E) gain of electrons or loss of H
B)
In the following reaction, when the equation is correctly balanced, what is the correct coefficient for H2?Fe(s) + HCl(aq) → FeCl3(aq) + H2(g) A) 1 B) 2 C) 3 D) 4 E) 5
C)
How many grams of N2 are produced from 100. g of NH3 in the following reaction? 4NH3(g) + 6NO(g) → 5N2(g) + 6H2O(l) A) 165 g B) 132 g C) 125 g D) 206 g E) 7.35 g
D)
How many grams of water will 100. grams of hydrogen peroxide (H2O2) produce? A) 3600 g B) 360. g C) 5.88 g D) 52.9 g E) 106 g
D)
In an oxidation-reduction reaction, the substance reduced always A) takes on oxygen atoms. B) shows a loss of electrons. C) gives up hydrogen atoms. D) shows a gain of electrons. E) becomes a charged species.
D)
In this reaction, what is the substance oxidized? Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g) A) chlorine B) zinc chloride C) hydrogen D) zinc E) oxygen
D)
Mg3N2 (s) + 6H2O(l) → 3Mg (OH)2 (s) + 2NH3 (g) When 36.0 g of H2O react, how many grams of NH3 are produced? A) 34.0 g B) 10.0 g C) 5.67 g D) 11.3 g E) 102 g
D)
One mole of neon atoms has a mass of A) 6.02 × 1023 grams. B) 14.0 g. C) 10.0 g. D) 20.2 g. E) 30.2 g.
D)
The following reaction takes place when an electric current is passed through water. It is an example of a ________ reaction. 2H2O → 2H2 + O2 A) combination B) single replacement C) dehydration D) decomposition E) double replacement
D)
What is the classification for this unbalanced reaction? Fe + HCl → FeCl3+ H2 A) dehydration B) combination C) decomposition D) single replacement E) double replacement
D)
What is the molar mass of sucrose (C12H22O11)? A) 29.0 g B) 50.2 g C) 210 g D) 342 g E) 182 g
D)
When 10.0 g of NH3 reacts, the actual yield of N2 is 8.50 g. What is the percent yield? 4NH3(g) + 6NO(g) → 5N2(g) + 6H2O(l) A) 85.0% B) 51.5% C) 20.6% D) 41.3% E) 8.5%
D)
2H2O2 → 2H2O + O2 How many moles of oxygen gas can 0.88 mole of hydrogen peroxide (H2O2) produce, if decomposition is complete? A) 0.50 mole B) 0.88 mole C) 1.8 moles D) 2.0 moles E) 0.44 mole
E)
Given the following equation, what is the correct form of the conversion factor needed to convert the number of moles of O2 to the number of moles of Fe2O3 produced?
E)
How many moles of iron are present in 3.15 × 1024 atoms of iron? A) 5.23 moles B) 1.90 moles C) 292 moles D) 0.523 moles E) 1.90 × 1048 moles
A)
In this reaction, what is the coefficient for calcium oxide? CaO(s) + CO2(g) → CaCO3(s) A) 1 B) 2 C) 3 D) 4 E) 5
A)
Mg3N2 (s) + 6H2O(l) → 3Mg (OH)2 (s) + 2NH3 (g) What is the correct form of the conversion factor needed to convert the number of moles of H2O to the number of moles of NH3 produced?
A)
When 85.0 g of CH4 are mixed with 160. g of O2 what is the maximum amount of CO2 that can be produced? CH4 + 2O2 → CO2 + 2H2O A) 2.50 moles B) 5.00 moles C) 5.31 moles D) 7.81 moles
A)
2Mg + O 2 → 2MgO2 The number of moles of oxygen gas needed to react with 4.0 moles of Mg is A) 1.0 mole. B) 2.0 moles. C) 3.0 moles. D) 4.0 moles. E) 6.0 moles.
B)
